Textbook-Integrated Guide to Educational Resources

TIGER

A Dramatic Classroom Demonstration of Limiting Reagent Using the Vinegar and Sodium Hydrogen Carbonate ReactionRomklao Artdej and Tienthong ThongpanchangThis demonstration, appropriate for high school chemistry level and recommended for a large classroom presentation, is designed to illustrate the concept of limiting reagent via a series of experiments in which increasing amounts of sodium bicarbonate are added to a fixed amount of vinegar is fixed until the volume of carbon dioxide generated remains constant. Artdej, Romklao; Thongpanchang, Tienthong. J. Chem. Educ.2008, 85, 1382.

A Simple Penny AnalysisNicholas C. Thomas and Stephen FaulkDescribes a simple procedure for determining the zinc composition of U.S. pennies in which the penny zinc core is dissolved in acid and the evolved hydrogen gas is collected by water displacement.Thomas, Nicholas C.; Faulk, Stephen. J. Chem. Educ.2008, 85, 817.

Scientific–Chemical Viewpoints Regarding Smoking: A Science Laboratory for AllRon BlonderThis article describes a lab that examines the acidity of cigarette smoke as well as solid particles and vapor phase substances found therein, and simulates the effects of smoking on the lungs. The aim of this activity is to expose adolescents to the scientific aspects of smoking and the relevance of chemistry in everyday life.Blonder, Ron. J. Chem. Educ.2008, 85, 248.

How Many Atomic Layers of Zinc Are in a Galvanized Iron Coating? Shui-Ping YangThis article describes a guided inquiry and problem solving experiment in which students use a novel gasometric assembly to determine the thickness and number of atomic layers of zinc coating on galvanized iron wires and nails.Yang, Shui-Ping. J. Chem. Educ.2007, 84, 1792.

Concept Maps for General Chemistry Boyd L. EarlTwo concept maps have been developed to represent the organization of the material in a first-semester general chemistry course. By providing these maps to students and referring to them in class, it is hoped that the instructor can assist students in maintaining a grasp of the "big picture" during the progress of the course.Earl, Boyd L. J. Chem. Educ.2007, 84, 1788.

Atomic Properties / Structure |

Gases |

Molecular Properties / Structure |

Stoichiometry |

Periodicity / Periodic Table

Geographical Information Systems (GIS) Mapping of Environmental Samples across College CampusesKathleen L. Purvis-Roberts, Harriet P. Moeur, and Andrew ZanellaIn this laboratory experiment, students take environmental samples (concentrations of nitrogen dioxide) and geospatial coordinates with a global position systems unit at various locations around campus, map their data on a geo-referenced map with geographical information systems software, and compare their results to those observed by governmental agencies.Purvis-Roberts, Kathleen L.; Moeur, Harriet P.; Zanella, Andrew. J. Chem. Educ.2007, 84, 1691.

Applications of Chemistry |

Atmospheric Chemistry |

Gases |

Laboratory Computing / Interfacing |

UV-Vis Spectroscopy

Carbon Dioxide FountainSeong-Joo Kang and Eun-Hee RyuThis article presents the development of a carbon dioxide fountain that, unlike the traditional ammonia fountain, is odorless and uses consumer chemicals. This experiment also allows students to see evidence of a gaseous reagent being consumed when a pressure sensor is available.Kang, Seong-Joo; Ryu, Eun-Hee. J. Chem. Educ.2007, 84, 1671.

Acids / Bases |

Consumer Chemistry |

Gases |

Laboratory Equipment / Apparatus |

Reactions

Incomplete Combustion of Hydrogen: Trapping a Reaction IntermediateBruce Mattson and Trisha HoetteIn this demonstration, a hydrogen flame is played across the face of an ice cube and the combustion is quenched in an incomplete state. The resulting solution contains a stable side-product, hydrogen peroxide, whose presence can be verified with two simple chemical tests.Mattson, Bruce; Hoette, Trisha. J. Chem. Educ.2007, 84, 1668.

Descriptive Chemistry |

Free Radicals |

Gases |

Molecular Properties / Structure |

Reactions |

Reactive Intermediates

A Fast Coulometric Estimation of Avogadro's NumberNicholas C. ThomasUsing simple materials found in any high school or college laboratory, an electrochemical method of determining Avogadro's number is presented.Thomas, Nicholas C. J. Chem. Educ.2007, 84, 1667.

Electrochemistry |

Gases

The Use of Limits in an Advanced Placement Chemistry CoursePaul S. Matsumoto, Jonathan Ring, and Jia Li (Lily) ZhuThis article describes the use of limits in topics usually covered in advanced placement or first-year college chemistry. This approach supplements the interpretation of the graph of an equation since it is usually easier to evaluate the limit of a function than to generate its graph.Matsumoto, Paul S.; Ring, Jonathan; Zhu, Jia Li (Lily). J. Chem. Educ.2007, 84, 1655.

Acids / Bases |

Equilibrium |

Gases |

Mathematics / Symbolic Mathematics |

Thermodynamics

Exception to the Le Châtelier PrincipleThomas R. HerrintonDisagreement regarding an apparent exception to the Le Chtelier principle involving the effects of nonideality on the direction in which the ammonia synthesis reaction shifts upon addition of infinitesimal and finite quantities of nitrogen at constant pressure and temperature. Herrinton, Thomas R. J. Chem. Educ.2007, 84, 1427.

Equilibrium |

Gases

Exception to the Le Châtelier PrincipleThomas R. HerrintonDisagreement regarding an apparent exception to the Le Chatelier principle involving the effects of nonideality on the direction in which the ammonia synthesis reaction shifts upon addition of infinitesimal and finite quantities of nitrogen at constant pressure and temperature. Herrinton, Thomas R. J. Chem. Educ.2007, 84, 1427.

What Are Students Thinking When They Pick Their Answer?Michael J. Sanger and Amy J. Phelps330 students were asked to answer a multiple-choice question concerning gas properties at the microscopic level and explain their reasoning. Of those who selected the correct answer, 80% provided explanations consistent with the scientifically accepted answer, while 90% of the students who picked an incorrect choice provided explanations with at least one misconception.Sanger, Michael J.; Phelps, Amy J. J. Chem. Educ.2007, 84, 870.

Gases |

Kinetic-Molecular Theory |

Phases / Phase Transitions / Diagrams |

Qualitative Analysis

Enthalpy of Vaporization and Vapor Pressures: An Inexpensive ApparatusRubin Battino, David A. Dolson, Michael R. Hall, and Trevor M. LetcherDescribes an inexpensive apparatus for the determination of the vapor pressure of a liquid as a function of temperature for the purpose of calculating enthalpy changes of vaporization. Also described are a simple air thermostat and an inexpensive temperature controller based on an integrated temperature sensor.Battino, Rubin; Dolson, David A.; Hall, Michael R.; Letcher, Trevor M. J. Chem. Educ.2007, 84, 822.

Where Did the Water Go? Boyle's Law and Pressurized Diaphragm Water TanksJames Brimhall and Sundar NagaBoyles law (PV is constant) provides mathematical insight into the workings of pressurized diaphragm tanks for storage of water pumped from underground wells, including predictions of the quantities of available water resulting from different initial conditions of water tank systems.Brimhall, James; Naga, Sundar. J. Chem. Educ.2007, 84, 425.

Job's Analysis of the Range of the "Dalton Syringe Rocket"Natalie Barto, Brandon Henrie, and Ed VitzAn apparatus for safely igniting fuel gas/oxygen mixtures in a syringe and measuring the distance that the syringe is propelled is presented. The distance (range) is analyzed by the method of continuous variation (Job's Method) to determine the stoichiometry of the reaction.Barto, Natalie; Henrie, Brandon; Vitz, Ed. J. Chem. Educ.2006, 83, 1505.

Gases |

Oxidation / Reduction |

Thermodynamics |

Stoichiometry

Teaching Physical Chemistry Experiments with a Computer Simulation by LabVIEWA. Belletti, R. Borromei, and G. InglettoThis article reports on a computer simulation developed with the software LabVIEW of the physical chemistry experiment regarding the vapor pressure measurements of a pure liquid as a function of temperature, as well as a system of data collecting that emphasizes the similarities between the virtual and real experiment.Belletti, A.; Borromei, R.; Ingletto, G. J. Chem. Educ.2006, 83, 1353.

Equilibrium |

Laboratory Computing / Interfacing |

Liquids |

Thermodynamics |

Gases |

Student-Centered Learning

Two "Gas-in-a-Bag" Reactions To Show the Predictive Power of the Relative AcidBase Strength ChartBrett CriswellDescribes a demonstration in which two different pairs of solid chemicals mixed in two different Ziploc bags in the presence of a small quantities of water react to produce gases. Students are informed that the reactions are BrnstedLowry acidbase type reactions and must determine which member in each pair will act as the acid and which as the base.Criswell, Brett. J. Chem. Educ.2006, 83, 1167.

Gas Permeability of PolymersJee-Yon LeeUndergraduate students can learn what causes the helium-inflated balloon to fall in a few days through the proposed experiment.Lee, Jee-Yon. J. Chem. Educ.2005, 82, 1472.

Gases |

Transport Properties

Gas Permeability of PolymersBruno LunelliThe recent article, Applying Chemical Potential and Partial Pressure Concepts To Understand the Spontaneous Mixing of Helium and Air in a Helium-Inflated Balloon, proposes a model of permeation untenable and in contradiction with correct statements present in the same text and consequently does not consider the material of which the investigated balloons are made.Lunelli, Bruno. J. Chem. Educ.2005, 82, 1471.

Gases |

Transport Properties

Gas Permeability of PolymersBruno LunelliBy studying a number of soft drinks with color but with or without phosphoric acid, the authors have determined that the required 20-fold dilution required in the Determination of Phosphorus in Cola Drinks is not to dilute the color but merely to place the sample within the calibration range of the analysis.Lunelli, Bruno. J. Chem. Educ.2005, 82, 1471.

A Passive Sampler for Determination of Nitrogen Dioxide in Ambient AirDan Xiao, Lianzhi Lin, Hongyan Yuan, Martin M. F. Choi, and Winghong ChanThis article describes the use of a passive sampler for detecting and collecting nitrogen dioxide, NO2, in ambient air. This device is based on microporous PTFE membranes that allow air samples to diffuse through and subsequently react with an absorbing reagent solution. The absorbance value of this reagent is proportional to the NO2 concentration in ambient air. It has been successfully applied to determine the NO2 concentrations in various sampling sites.Xiao, Dan; Lin, Lianzhi; Yuan, Hongyan; Choi, Martin M. F.; Chan, Winghong. J. Chem. Educ.2005, 82, 1231.

Calibration |

Membranes |

UV-Vis Spectroscopy |

Amines / Ammonium Compounds |

Coordination Compounds |

Gases |

Laboratory Equipment / Apparatus |

Nonmajor Courses |

Quantitative Analysis

A Note on Dalton's Law: Myths, Facts, and ImplementationRonald W. Missen and William R. SmithThe treatment of Dalton's law for gas mixtures commonly includes the improper designation "Dalton's law of partial pressures", rather than the correct "Dalton's law of additivity of (pure component) pressures". It also identifies the pure component pressure as the partial pressure, although these are only numerically equal for a mixture of ideal gases. The situation is clarified by examination of an appropriate statement of the law and definitions, eventually in operational form with reference to mixtures of nonideal gases.Missen, Ronald Wi.; Smith, William R. J. Chem. Educ.2005, 82, 1197.

Thermodynamics |

Gases

Some Insights Regarding a Popular Introductory Gas Law ExperimentEd DePierro and Fred GarafaloThis paper alerts readers to a potential source of error in one approach to the Dumas method as it is often practiced in introductory chemistry laboratories. The room-temperature vapor pressures of volatile compounds that might be considered as unknowns for the experiment lead to determined molar masses that are too low. The greater the vapor pressure of the compound, the lower the determined molar mass will be, when compared to the accepted value. DePierro, Ed; Garafalo, Fred. J. Chem. Educ.2005, 82, 1194.

Gases |

Laboratory Equipment / Apparatus |

Phases / Phase Transitions / Diagrams |

Physical Properties

Steel Wool and Oxygen: A Look at KineticsJames Gordon and Katherine ChanceyAn experimental method is described to study the kinetics of the reaction of the iron in steel wool with molecular oxygen. A calculator-based data collection system is used with an oxygen gas sensor to determine the order of the reaction with respect to oxygen. Using the graphical method, students determine that the reaction follows first-order kinetics with respect to oxygen. Gordon, James; Chancey, Katherine. J. Chem. Educ.2005, 82, 1065.

Atmospheric Chemistry |

Gases |

Kinetics |

Oxidation / Reduction

Greenhouse Gases and Non-gray BehaviorJ. C. JonesGreenhouse gases feature in many courses in applied chemistry as well as in courses on environmental science, atmospheric chemistry, and so on. We hear a great deal about such matters from the media. A more classical topic which first-year chemistry students will learn about in the physical chemistry component of their program is the black body concept and the StefanBoltzmann law. Recently in teaching about greenhouse gases to MSc students I have thought of a link between the topical and classical matters that is pedagogically interesting and might be of value to others teaching in this subject area.Jones, J. C. J. Chem. Educ.2005, 82, 837.

Atmospheric Chemistry |

Gases

Applying Chemical Potential and Partial Pressure Concepts To Understand the Spontaneous Mixing of Helium and Air in a Helium-Inflated BalloonJee-Yon Lee, Hee-Soo Yoo, Jong Sook Park, Kwang-Jin Hwang, and Jin Seog KimIn developing this laboratory, our initial motivation for the analysis of gases in a balloon was to answer simple and basic questions, such as, Why does a helium-charged balloon left in the air always drop in a few days? Is leakage of helium the only cause of the drop? What is the composition of the gas in the balloon when it falls after deflation? Students were intrigued by these questions, too, as they analyzed the variation over time in the composition in a balloon inflated with helium. Using the concepts of partial pressure and chemical potential, the laboratory experiment described effectively investigates the diffusion process and the behavior of gas molecules for teaching these concepts in general and physical chemistry. Lee, Jee-Yon; Yoo, Hee-Soo; Park, Jong Sook; Hwang, Kwang-Jin; Kim, Jin Seog. J. Chem. Educ.2005, 82, 288.

Transport Properties |

Gases |

Mass Spectrometry |

Quantitative Analysis

The Determination of the Percent of Oxygen in Air Using a Gas Pressure SensorJames Gordon and Katherine ChanceyA new detection method is applied to a classic experiment in which gaseous atmospheric oxygen in a test tube is reacted with the iron in steel wool to produce rust. A gas pressure sensor interfaced to a calculator-based data collection system was used to measure the percent of oxygen in the air as the reaction proceeded. The results from the calculator-based experiment were compared to the results from a more traditional water-measurement experiment. The average percent of oxygen obtained using the calculator system was 19.4  0.4%. Gordon, James; Chancey, Katherine. J. Chem. Educ.2005, 82, 286.

Atmospheric Chemistry |

Gases |

Oxidation / Reduction |

Reactions

Fractional Distillation of Air and Other Demonstrations with Condensed GasesMaria Oliver-Hoyo and William L. Switzer, IIIThis demonstration builds upon the commonly performed liquefaction of air not only to show the presence of nitrogen and oxygen, but also the presence of two other components, carbon dioxide and water. Several extensions are suggested: one to show boiling point elevation in solution and another to show the elevation of both boiling point and sublimation point with pressure. No special apparatus is required permitting presentations to audiences in a variety of settings. These demonstrations give the opportunity to discuss properties of gases, solution chemistry, and phase equilibria.Oliver-Hoyo, Maria; Switzer, William L., III. J. Chem. Educ.2005, 82, 251.

Gases |

Qualitative Analysis |

Atmospheric Chemistry |

Phases / Phase Transitions / Diagrams |

Separation Science

A Methane Balloon Inflation ChamberCurtis J. Czerwinski and Tanya J. CordesWhile several lecture demonstrations are possible using methane-filled balloons, it is often inconvenient to prepare these balloons since the pressure from standard laboratory and lecture hall gas nozzles is too low. As a solution to this problem, a methane balloon inflation chamber, prepared from a translucent 3.5-gallon pail and an aspirator or house-vacuum, provides an inexpensive and convenient method for inflating balloons in laboratories or lecture halls. Prepared in this way, methane-filled balloons can be used to demonstrate the effects of vacuum, the lifting power of low-density gases, and the explosive combustion of methane. Czerwinski, Curtis J.; Cordes, Tanya J. J. Chem. Educ.2005, 82, 248.

Alkanes / Cycloalkanes |

Calorimetry / Thermochemistry |

Gases |

Oxidation / Reduction |

Reactions

On the Buoyancy of a Helium-Filled BalloonJohn E. HarrimanIt is shown by expansion of the exponential in the barometric formula that the forces due to pressure acting on a balloon are of the form (PV/RT)Mg and that results agree with those suggested by Archimedes principle. Einstein's equivalence principal provides an answer to what balloons will do in an accelerated car. Harriman, John E. J. Chem. Educ.2005, 82, 246.

Campbell's Rule for Estimating Entropy ChangesWilliam B. JensenIn a recent article Norman Craig has proposed the rule-of-thumb that the approximate value of the entropy of reaction is related to the net moles of gas consumed or generated in the reaction .Jensen, William B. J. Chem. Educ.2004, 81, 1570.

Gases |

Thermodynamics

Construction of a Small-Scale and Low-Cost Gas ApparatusLise Kvittingen and Richard VerleyThis article describes how to construct an apparatus for gas production from disposable polyethene pipets and polypropene microcentrifuge tubes. Heat is used to form the plastics into appropriate shapes. A stand from floral wire is also presented. The assembly has an open interface and is possible to modify. This construction suits various grades and curricula and can easily be integrated into different topics. Kvittingen, Lise; Verley, Richard. J. Chem. Educ.2004, 81, 1339.

Laboratory Equipment / Apparatus |

Microscale Lab |

Gases

Water in the AtmosphereJoel M. KauffmanNone of eight college-level general chemistry texts gave a mean value for water in the atmosphere, despite its being the third most prevalent constituent at about 1.5% by mass as vapor and about 2% if clouds and ice crystals are included. The importance of water as a greenhouse gas was omitted or marginalized by five of the eight texts. An infrared spectrum of humid air was determined to demonstrate that water vapor, because of its higher concentration, was more absorptive than carbon dioxide. The cooling effect of clouds, or other influences on the Earth's albedo, were not mentioned in most of the texts. These pervasive errors should be corrected in new or future editions of textbooks. Kauffman, Joel M. J. Chem. Educ.2004, 81, 1229.

Atmospheric Chemistry |

Gases |

Green Chemistry |

IR Spectroscopy

Mass Spectrometry for the MassesJared D. Persinger, Geoffrey C. Hoops, and Michael J. SamideIn this article, we describe an experiment for an introductory chemistry course that incorporates the use of mass spectrometry for sample analysis. Several different air samples are collected that represent various chemical processes, and the composition of the air sample is predicted on the basis of known chemical principles. A gas chromatograph-mass spectrometer is used to analyze these samples, and the relative quantities of nitrogen, oxygen, carbon dioxide, water, and argon are calculated. On the basis of the data, the hypothesized sample composition is validated. Persinger, Jared D.; Hoops, Geoffrey C.; Samide, Michael J. J. Chem. Educ.2004, 81, 1169.

The Decomposition of Zinc Carbonate: Using Stoichiometry To Choose between Chemical FormulasStephen DeMeoTo determine which formula corresponds to a bottle labeled "zinc carbonate", students perform qualitative tests on three of zinc carbonate's decomposition products: zinc oxide, carbon dioxide, and water. Next students make quantitative measurements to find molar ratios and compare them with the coefficients of the balanced chemical equations. This allows the correct formula of zinc carbonate to be deduced. DeMeo, Stephen. J. Chem. Educ.2004, 81, 119.

Carbon Dioxide Flooding: A Classroom Case Study Derived from Surgical PracticeRobert C. KerberThe surgical opening in open-heart surgery is often flooded with carbon dioxide gas to avoid air embolisms when the heart is closed and restarted. This practice can be used in chemistry courses to illustrate concepts of gas density, solubility, and acidbase equilibria, including buffering.Kerber, Robert C. . J. Chem. Educ.2003, 80, 1437.

Acids / Bases |

Aqueous Solution Chemistry |

Gases |

Medicinal Chemistry |

Nonmajor Courses |

Applications of Chemistry

Why Does a Helium-Filled Balloon "Rise"?Richard W. RametteThe article is a lighthearted, conversational exploration of the microscopic basis for Archimedes principle. The principle is discussed in terms of molecular collisions and density gradients in a gravitational field. Ramette, Richard W. J. Chem. Educ.2003, 80, 1149.

Just Breathe: The Oxygen Content of Air JCE Editorial StaffStudents estimate the percent oxygen (volume) in air using steel wool in a test tube that is inverted in a beaker of water. Oxygen in the trapped air reacts with iron to form rust, and the water level rises inside the test tube; within 30-45 minutes, the majority of oxygen is consumed.JCE Editorial Staff. J. Chem. Educ.2001, 78, 512A.

Electrochemistry |

Gases |

Oxidation / Reduction

Sink or Swim: The Cartesian DiverK. David PinkertonCartesian divers are a quick and simple way to illustrate relationships among pressure, volume, temperature, and buoyancy. The Activity could be used in connection with the concepts of gases and liquids and discussions of Boyle's, Charles's, and the ideal gas laws.Pinkerton, K. David. J. Chem. Educ.2001, 78, 200A.

Determination of the Universal Gas Constant, R. A Discovery LaboratoryDavid B. Moss and Kathleen CornelyDiscovery laboratory in which groups of students collect oxygen, hydrogen, and nitrogen gas over water and determine the value of the universal gas constant, R, using the ideal gas law.Moss, David B.; Cornely, Kathleen. J. Chem. Educ.2001, 78, 1260.

Gases

"Experiment with a Candle" without a CandleDusan Krnel and Sasa A. GlazarDrawing water up into an inverted container without using the candle to demonstrate that the popular explanation for this phenomenon is flawed.Krnel, Dusan; Glazar, Sasa A. J. Chem. Educ.2001, 78, 914.

Are Fizzing Drinks Boiling? A Chemical Insight from Chemical Education ResearchAlan GoodwinThe suggestion that fizzing drinks are examples of liquids boiling at room temperature has proved to be controversial among both chemists and chemical educators. This paper presents a case for believing this everyday system to be a good example of a boiling solution and the consequent separation of carbon dioxide from the solution to exemplify fractional distillation. Goodwin, Alan. J. Chem. Educ.2001, 78, 385.

Aqueous Solution Chemistry |

Kinetic-Molecular Theory |

Equilibrium |

Gases |

Solutions / Solvents |

Phases / Phase Transitions / Diagrams

A Simple Laboratory Experiment for the Determination of Absolute ZeroMyung-Hoon Kim, Michelle Song Kim, and Suw-Young LyA novel method that employs a remarkably simple and inexpensive apparatus and is based on the extrapolation of the volume of a given amount of dry air to zero volume after a volume of air trapped inside a 10-mL graduated cylinder is measured at various temperatures.Kim, Myung-Hoon; Kim, Michelle Song; Ly, Suw-Young. J. Chem. Educ.2001, 78, 238.

A Novel Experiment for Fast and Simple Determination of the Oxygen Content in the AirMetodija Najdoski and Vladimir M. PetrusevskiThe reaction between nitric oxide (NO) and oxygen is used for determination of the oxygen content in the air. The nitrogen dioxide thus produced is dissolved in water. The volume decrease of the gas enables quick and accurate enough determination of the O2 content. The results of 20 measurements give %O2 = 21.04  0.63. Najdoski, Metodija; Petrusevski, Vladimir M. J. Chem. Educ.2000, 77, 1447.

Potentiometric Determination of CO2 Concentration in the Gaseous Phase: Applications in Different Laboratory ActivitiesEduardo Cortón, Santiago Kocmur, Liliana Haim, and Lydia GalagovskyThe first lab comprises the calibration of a CO2 potentiometric detector with gas mixtures. The CO2 and CO2-free air required for the gaseous samples are produced in the lab by an inexpensive and simple apparatus. In the second lab, the CO2 potentiometric device is used to measure CO2 uptake and release during different metabolic processes. Cortón, Eduardo; Kocmur, Santiago; Haim, Liliana; Galagovsky, Lydia. J. Chem. Educ.2000, 77, 1188.

Electrochemistry |

Gases |

Quantitative Analysis |

Metabolism

A New Approach to Teaching Introductory Science: The Gas ModulePamela Mills, William V. Sweeney, Robert Marino, and Sandra ClarksonA lecture/laboratory module about the behavior of gases that is designed to expose students to the process of scientific discovery, not to teach the gas laws per se. The topic of gases is only the medium used to illustrate other important aspects of physical science: how to process experimental data and reduce it to symbolic mathematical relationships, how to evaluate the reliability of experimental data, and how to view the relationship between experimental data and scientific models. Mills, Pamela A.; Sweeney, William V.; Marino, Robert; Clarkson, Sandra. J. Chem. Educ.2000, 77, 1161.

Gases

Paradoxes, Puzzles, and Pitfalls of Incomplete Combustion DemonstrationsEd VitzPaper is burned in a closed container containing sufficient oxygen to consume all the paper. Paradoxically, the flame expires while half of the paper remains. This demonstrates that thermodynamics or stoichiometry is insufficient to explain everyday chemical processes, and that kinetics is often necessary. The gases in the container are analyzed by GC before and after combustion, and the results are examined in detail. Vitz, Ed. J. Chem. Educ.2000, 77, 1011.

Gas Me Up, or, A Baking Powder DiverHenry R. Derr, Tricia Lewis, and Bretton J. DerrIn this procedure, a pipet that repeatedly submerges and rises to the surface in a tub of water is produced from a beral pipet and baking powder. The procedure works well in outreach activities with children aged 4 to 40 and beyond.Derr, Henry R.; Lewis, Tricia; Derr, Bretton J. J. Chem. Educ.2000, 77, 171.

Acids / Bases |

Gases

Determination of the Fundamental Electronic Charge via the Electrolysis of WaterBrittany Hoffman, Elizabeth Mitchell, Petra Roulhac, Marc Thomes, and Vincent M. StumpoIn an illuminating experiment suitable for secondary school students, a Hoffman electrolysis apparatus is employed to determine the fundamental electronic charge. The volume and pressure of hydrogen gas produced via the electrolysis of water during a given time interval are measured. Hoffman, Brittany; Mitchell, Elizabeth; Roulhac, Petra; Thomes, Marc; Stumpo, Vincent M. J. Chem. Educ.2000, 77, 95.

Atomic Properties / Structure |

Electrochemistry |

Gases |

Molecular Properties / Structure

Henry's Law and Noisy KnucklesDoris R. KimbroughPresented here is the application of Henry's law to the noise associated with "cracking" knuckles. Gases dissolved in the synovial fluid in joints rapidly come out of solution as the joint is stretched and pressure is decreased. This "cavitation" produces a characteristic noise. Kimbrough, Doris R. J. Chem. Educ.1999, 76, 1509.

Relative HumidityR. Bruce MartinDaily we hear reports of relative humidity, yet most students remain unfamiliar with its import. This short article defines and describes the concept at several levels. A new, general interest, isobaric plot directly indicates the dependence of relative humidity on temperature. Martin, R. Bruce. J. Chem. Educ.1999, 76, 1081.

Consumer Chemistry |

Gases |

Nonmajor Courses |

Water / Water Chemistry |

Atmospheric Chemistry

A More Dramatic Container to Crush by Atmospheric PressureRobert D. Meyers and Gordon T. YeeThe familiar demonstration of collapsing a can by filling it with water vapor and then sealing it and allowing it to cool is improved by performing it with a 20-L steel solvent drum instead. Meyers, Robert D.; Yee, Gordon T. J. Chem. Educ.1999, 76, 933.

Gases |

Phases / Phase Transitions / Diagrams

Ammonia Can CrushEd VitzWhen a 12-oz aluminum soft drink can filled with ammonia or hydrogen chloride gas is inverted and dipped into water, the rapidly dissolving gas evacuates the can and the can is crushed before water can be drawn into it. This demonstrates, among other things, the remarkable strength of hydrogen bonds. Vitz, Ed. J. Chem. Educ.1999, 76, 932.

Noncovalent Interactions |

Gases |

Solutions / Solvents |

Hydrogen Bonding

The Persistence of the Candle-and-Cylinder MisconceptionJames P. Birk and Anton E. LawsonThere is a persistent misconception that when a lighted candle is supported in a container of water and a closed cylinder is lowered over the candle, the candle is extinguished after a time by complete consumption of the oxygen in the cylinder, with a volume change corresponding to the amount of oxygen in the air. This misconception has appeared in the literature periodically for many years. Here, we present a number of experiments that refute this misconception.Birk, James P.; Lawson, Anton E. J. Chem. Educ.1999, 76, 914.

Gases |

Atmospheric Chemistry |

Quantitative Analysis |

Reactions

The Methane BalloonWalter H. Corkern and Elvin Hughes Jr.The objectives are (i) to describe a novel method of inflating a balloon with methane, (ii) to show that methane is lighter than air, and (iii) to demonstrate the flammability of methane. Corkern, Walter H.; Hughes, Elvin, Jr. J. Chem. Educ.1999, 76, 794.

Gases |

Oxidation / Reduction |

Reactions

Both Nylon and PET Fibers Burn Continuously under Atmospheric ConditionsShouei Fujishige, Nagako Maebashi, and Mizue MiyauchiIn contrast to the descriptions in many textbooks, it was confirmed by taking two series of photographs that both nylon and PET fibers burn continuously even after the ignition flame has been removed. The photographs also show that a small spherical fire ball forms and occasionally leaves from the flame.Fujishige, Shouei; Maebashi, Nagako; Miyauchi, Mizue. J. Chem. Educ.1999, 76, 793.

Consumer Chemistry |

Materials Science |

Gases |

Laboratory Management

Pressure and StoichiometryCharles E. Roser and Catherine L. McCluskeyThis experiment determines the stoichiometry of the reaction of a carbonate or hydrogen carbonate and HCl by measuring the pressure of the CO2 produced using a Vernier pressure sensor, TI CBL interface, and a TI-82/83 graphing calculator. Various amounts of the carbonate are reacted with a constant amount of HCl. Roser, Charles E.; McCluskey, Catherine L. J. Chem. Educ.1999, 76, 638.

Stoichiometry |

Gases |

Laboratory Computing / Interfacing

A Demonstration of Ideal Gas Principles Using a FootballWilliam D. Bare and Lester AndrewsA class demonstration and cooperative learning activity in which the ideal gas law is applied to determine the volume of a football is described. The mass of an air-filled football is recorded at two or more pressures, and students are asked to use these data to solve problems involving the volume, pressure, and mass of the football and the molecular weight of the gas in the ball.Bare, William D.; Andrews, Lester. J. Chem. Educ.1999, 76, 622.

The Ammonia Smoke Fountain: An Interesting Thermodynamic AdventureM. Dale AlexanderThe ammonia smoke fountain demonstration utilizes a modification of the apparatus used in the standard ammonia fountain. The modification allows for the introduction of hydrogen chloride gas into a flask of ammonia rather than water. The flow rate of hydrogen chloride gas into the flask in the smoke fountain is not constant, but periodic; that is, the smoke puffs from the end of the tube. This unexpected behavior elicits an interesting thermodynamic explanation.Alexander, M. Dale. J. Chem. Educ.1999, 76, 210.

Acids / Bases |

Gases |

Thermodynamics |

Reactions |

Stoichiometry |

Precipitation / Solubility

The Fizz Keeper, a Case Study in Chemical Education, Equilibrium, and KineticsReed HowaldThe chemistry of the loss of carbonation from carbonated beverages on storage is considered. Increasing the pressure of CO2(g) will restore carbonation, but an increase in pressure adding air should not affect the equilibria. It can and does, however, affect the kinetics-the rate at which a new equilibrium is established. Thus the Fizz Keeper is effective for storage of resealed pop containers for hours, but not for periods of weeks or months. Howald, Reed. J. Chem. Educ.1999, 76, 208.

A Precise Method for Determining the CO2 Content of Carbonate MaterialsDonald L. Pile, Alana S. Benjamin, Klaus S. Lackner, Christopher H. Wendt, and Darryl P. ButtThe design and use of a buret apparatus for CO2 gas capture and mass determination are described. The derivation of a comprehensive equation to determine the CO2 mass and percent carbonation of the material is outlined. Experimental factors such as temperature and pressure, including elevation effects, and apparatus parameters are discussed and incorporated into one general equation.Pile, Donald L.; Benjamin, Alana S.; Lackner, Klaus S.; Wendt, Christopher H.; Butt, Darryl P. J. Chem. Educ.1998, 75, 1610.

Laboratory Equipment / Apparatus |

Gases |

Quantitative Analysis

Generating Water-Soluble Noxious Gases: An Overhead Projector DemonstrationSally Solomon, Maria Oliver-Hoyo, and Chinhyu HurA simple, inexpensive apparatus to generate and collect water-soluble noxious gases as an overhead projector demonstration can be made from two small beakers and a Petri dish. The detection and generation of sulfur dioxide and nitrogen dioxide are described. Solomon, Sally; Oliver-Hoyo, Maria; Hur, Chinhyu. J. Chem. Educ.1998, 75, 1581.

Gases |

Oxidation / Reduction |

Carbohydrates |

Toxicology

Gas Experiments with Plastic Soda BottlesPatrick Kavanah and Arden P. ZippThe construction and use of a new device to study gases is described. The device, which is made from a plastic soda bottle and an automobile tire valve, can be used to demonstrate that air has mass, find the mass of the "evacuated" device, determine the molar mass of air and other gases, investigate the pressure-volume relationship, and build a cloud chamber. Kavanah, Patrick; Zipp, Arden P. J. Chem. Educ.1998, 75, 1405.

A Simple, Transparent Fume HoodJohn FredericksAn inexpensive transparent fume hood can be constructed from a clear-plastic two-liter soft drink bottle that is cut just above the base. A length of vacuum tubing is secured to the opening of the bottle using black electrical tape. The tubing is then connected to a water aspirator.Fredericks, John. J. Chem. Educ.1998, 75, 1299.

Chemistry in the Public DomainOdom, John L.Mixtures of ammonia-air and methylene chloride-air can be explosive.Odom, John L. J. Chem. Educ.1998, 75, 1087.

Gases

Experimentally Determining the Molar Mass of Carbon Dioxide Using a Mylar BalloonBarbara Albers Jackson and David J. CrouseThe molar mass of carbon dioxide was experimentally determined using a Mylar balloon. Mylar balloons are lightweight, have a fixed definite volume, and require minimal additional pressure for inflation. Using the Ideal Gas Equation, the number of moles of air in the balloon was calculated. Jackson, Barbara Albers; Crouse, David J. J. Chem. Educ.1998, 75, 997.

Gases |

Physical Properties

Thermal Physics (and Some Chemistry) of the AtmosphereStephen K. LowerAn exploration of how the temperature of the atmosphere varies with altitude can serve as a useful means of illustrating some important principles relating to the behavior of gases and to the absorption and transformation of radiant energy. Lower, Stephen K. J. Chem. Educ.1998, 75, 837.

Atmospheric Chemistry |

Gases

Vapor Pressure Lowering by Nonvolatile SolutesGavin D. PeckhamThis short article highlights a fundamental error that is entrenched in introductory chemistry textbooks. It is true that the addition of a nonvolatile solute causes a lowering in the vapor pressure of a solution. The error lies in attributing this vapor pressure lowering to the "blocking" of surface sites by nonvolatile particles. This is a totally fallacious argument for a number of reasons and the true explanation is to be found in the entropy changes that occur as a nonvolatile solute is added to a solution. Peckham, Gavin D. J. Chem. Educ.1998, 75, 787.

Formation and Dimerization of NO2 A General Chemistry ExperimentApril D. Hennis, C. Scott Highberger, and Serge Schreiner*A general chemistry experiment which illustrates Gay-Lussac's law of combining volumes. Students are able to determine the partial pressures and equilibrium constant for the formation and dimerization of NO2. The experiment readily provides students with data that can be manipulated with a common spreadsheet. Hennis, April D.; Highberger, C. Scott; Schreiner, Serge. J. Chem. Educ.1997, 74, 1340.

Gases |

Equilibrium |

Quantitative Analysis |

Stoichiometry

Graham's Law and Perpetuation of ErrorStephen J. HawkesGrahams Laws of effusion and diffusion are used in recent articles for traditional experiments to which they do not in fact apply and for which they give the wrong answer.Hawkes, Stephen J. J. Chem. Educ.1997, 74, 1069.

A U-Tube Experiment To Discover the Curve in Boyle's LawThomas G. Richmond and Amy ParrA discovery-style experiment is described to enable introductory chemistry students to determine the pressure versus volume behavior of a gas over a wide pressure range to "discover" Boyle's Law. Richmond, Thomas G.; Parr, Amy. J. Chem. Educ.1997, 74, 414.

Gases |

Laboratory Equipment / Apparatus

A Simple Boyle's Law ExperimentDon L. LewisStudent-conducted experiments over a range of pressures from about 14 psi to about 120 psi can safely and accurately be made utilizing a 60 ml syringe and an ordinary bathroom scale. No pressure gauge is required and no value for initial pressure in the syringe (near atmospheric pressure) need be assumed. Lewis, Don L. J. Chem. Educ.1997, 74, 209.

Gases

Egg in the Bottle (2)Moran, MichaelThe cause of the pressure drop in the bottle is due to the cooling of high-temperature gases.Moran, Michael J. Chem. Educ.1996, 73, A189.

Gases

Egg in the Bottle (1)DeLorenzo, RonaldThe cooling of gas and the condensation of water vapor must be considered in addition to the loss of oxygen in reducing the pressure inside the glass bottle.DeLorenzo, Ronald J. Chem. Educ.1996, 73, A188.

Gases

The Use of PTFE Membranes for the Construction of Semimicroscale Gas ReactorsSchallies, Michale; Schnelle, Hans-Otto; Kunze, KlausThe membranes are employed to separate reaction compartments, where gas-evolving reactions take place, from solutions of reagents needed for qualitative or quantitative determinations of the gases. The PTFE membranes allow free flow of gases while they prevent the passage of water.Schallies, Michale; Schnelle, Hans-Otto; Kunze, Klaus J. Chem. Educ.1996, 73, A128.

Gases |

Qualitative Analysis |

Quantitative Analysis |

Laboratory Equipment / Apparatus |

Microscale Lab

Four Programs for Windows: Abstract of Volume 4D, Number 2: Alkanes in MotionJae Hyun KimAlkanes in Motion depicts the molecular motion of hydrocarbons in the gas phase. Four animations from the collection are presented here. These four animations consist of two animations each of hexane and octadecane, one animation calculated to show translational motion and one to show vibrational motion. Kim, Jae Hyun. J. Chem. Educ.1996, 73, 1079.

Molecular Modeling |

Alkanes / Cycloalkanes |

Molecular Properties / Structure |

Gases

Notes on Vapor Pressure Equilibria MeasurementsAlbert G. Krieger, John W. HendersonFreshman students at our institution use manometers and 24/40 ground-glass distillation apparatus (abandoned by our organic chemistry classes) to measure boiling points at reduced pressures. We have found that the availability of state-of-the-art equipment need not limit the ability to teach and demonstrate fundamental principlesKrieger, Albert G.; Henderson, John W. J. Chem. Educ.1996, 73, 1039.

Gases |

Physical Properties

Oxygen from Hydrogen Peroxide: An Experimental ModificationJames H. Burness This paper describes a simple modification to the generation of oxygen gas experiment which eliminates the need for a pencil coated with petroleum jelly and dry yeast. This elimination not only prevents falling pieces of yeast from prematurely starting the reaction, but at the same time makes the reaction faster and simplifies cleanup.J. Chem. Educ.1996, 73, 851.

SIRS: Simulations and Interactive Resources, IIIMartin, John S.Simulations and Interactive Resources (SIRs) are designed to support interactive lectures in introductory chemistry. This third issue of SIRs includes five new SIRs as well as updated and final versions of all previously published SIRs.Martin, John S. J. Chem. Educ.1996, 73, 722.

A Novel Approach to Teaching Electrochemical PrinciplesPaul Krause and Jerry ManionTo demonstrate that work may be done by a chemical reaction, a reaction producing a gas is carried out in a large, closed syringe. As the gas is generated, the syringe plunger is forced out.Krause, Paul; Manion, Jerry. J. Chem. Educ.1996, 73, 354.

The Solubility of Gases in LiquidsL. H. Holmes, Jr.This short article addresses the solubility of gases in liquids. It describes the confusion that appears in some general chemistry textbooks concerning the qualitative dependence of solubility on temperature for gases and offers an opinion on the subject. Holmes, L. H., Jr. J. Chem. Educ.1996, 73, 143.

The Environmental Chemistry of Trace Atmospheric GasesWilliam C. TroglerInformation regarding the composition of trace gases in the Earth's atmosphere, changes in these amounts, their sources, and potential future impact on the environment.Trogler, William C. J. Chem. Educ.1995, 72, 973.

The Tube-in-Tube Solution for Gas GenerationArnaiz, Francisco J.Simple apparatus using a magnetic stir bar for adding a liquid reactant to a solid when the volume of the gas produced by the reaction must be determined.Arnaiz, Francisco J. J. Chem. Educ.1995, 72, 572.

A simple demonstration of the law of combining volumes DuPre, Donald B.This demonstration is based on the reaction of two volumes of nitric oxide reacting with one volume of molecular oxygen to produce two volumes of nitrogen dioxide.DuPre, Donald B. J. Chem. Educ.1993, 70, 849.

Gases

Measurement scales: Changing Celsius to Kelvin is not just a unit conversion Nordstrom, Brian H.The key to understanding the difference between Celsius and Kelvin lies in the different types of measurement scales. Students may have an easier time manipulating equations (such as gas laws) if they knew the difference between these scales.Nordstrom, Brian H. J. Chem. Educ.1993, 70, 827.

Revealing the secret of the Arctic bomb Pearson, Earl F.Arctic bombs and hurricanes can appear to be contradictory to gas law concepts commonly taught to chemistry students. While these phenomena can be explained as applications of simple gas laws, the explanations can be more effective if an apparent contradiction is drawn between students' understanding and the observed pressure-temperature relationship in these two examples.Pearson, Earl F. J. Chem. Educ.1993, 70, 315.

Determining the thermal expansion coefficient of gasesLehmann, Jochen K.The authors improved the design of the apparatus and extended the experimental task on a recently published experiment for determining the zero point of the absolute temperature scale.Lehmann, Jochen K. J. Chem. Educ.1992, 69, 943.

Fast molecular motionKnox, KerroA demonstration that shows that molecules do indeed move very fast and over long distances in a short time when nothing is in the way.Knox, Kerro J. Chem. Educ.1992, 69, 574.

A simple generator for common gases at atmospheric pressureElsworth, John F.The current high cost of either a Kipps generator for producing hydrogen sulfide in the undergraduate laboratory, or of the bottled gas, led the writer to construct a simple, economical and efficient generator for use in a laboratory fitted with an efficient fume hood.Elsworth, John F. J. Chem. Educ.1992, 69, 419.

Gases |

Laboratory Equipment / Apparatus

Gas chamber stoichiometry Hunter, Norman W.; Wilkins, Curtis C.; Pearson, Earl F.Most students know that HCN is used in gas chambers, they may not know however that HCN is produced in the burning of carpets, draperies, clothing and other textiles made of polyacrylonitrile.Hunter, Norman W.; Wilkins, Curtis C.; Pearson, Earl F. J. Chem. Educ.1992, 69, 389.

Vapor pressure demonstrations using a butane lighterDelumyea, R. DelThe concept of the change of state of matter and particularly the volatitlity of liquids is an important concept taught in introductory chemistry courses.Delumyea, R. Del J. Chem. Educ.1992, 69, 321.

Gases |

Physical Properties |

Liquids |

Phases / Phase Transitions / Diagrams

An "egg-splosive" demonstration.Becker, Robert.The following demonstration uses an egg to demonstrate the explosive power of a combustible gaseous mixture.Becker, Robert. J. Chem. Educ.1992, 69, 229.

Gases

Demonstrations with red cabbage indicator Fortman, John J.; Stubbs, Katherine M.This paper extends the use of the red cabbage extract into demonstrations that illustrate the acidic or basic nature of solutions of gases and gives suggestions for modifications to project the beautiful range of colors and shades for better viewing in large lecture halls.Fortman, John J.; Stubbs, Katherine M. J. Chem. Educ.1992, 69, 66.

Does a one-molecule gas obey Boyle's law?Rhodes, GailBecause the kinetic molecular theory provides a plausible explanation for the lawful behavior of gases, it should be treated in enough depth to show students that the theory accounts for all of the important aspects of ideal gas behavior.Rhodes, Gail J. Chem. Educ.1992, 69, 16.

Use of liquid oxygen to support combustion Sullivan, Dan M.Production, procedure, and safety of demonstrations involving liquid nitrogen in order to demonstrate: Charles' Law, production and properties of liquid oxygen, effects of concentration on reactions and reaction rates, liquefaction and boiling of oxygen kindling temperature, reactions between substances in two different states of matter, and comparison of partial and complete combustion.Sullivan, Dan M. J. Chem. Educ.1991, 68, 1036.

A miniature hot air balloon and Charles's lawDeese, William C.Heating the air in a tissue paper balloon using a Merker burner and flying it up and down a guided wire in the classroom.Deese, William C. J. Chem. Educ.1990, 67, 672.

Questions from a can of PepsiMitchell, TonyA can of Pepsi can be the starting point of countless chemistry questions that students can relate to. The author encourages other instructors to think about helping students understand chemistry as it relates to contemporary society.Mitchell, Tony J. Chem. Educ.1988, 65, 1070.

An alternative to using the PV = nRT equation Desmarais, GeorgeThis author shares his application of the factor-label method to solving gas problems which involves using the ideal gas constant as the starting point in the relationship.Desmarais, George J. Chem. Educ.1988, 65, 392.

Control of variables and the conservation of matterGiachino, Gary G.Demonstrates the conservation of matter, but its main value lies in its illustration of the need to control variables and the difficulty this may entail - particularly if a variable is "hidden"; uses a burning candle in a glass flask.Giachino, Gary G. J. Chem. Educ.1987, 64, 353.

Interstellar chemistryCarbo, R.; Ginebreda, A.Surveys some of the features that characterize interstellar chemistry, particularly the composition of the interstellar medium and the nature of the changes that occur there.Carbo, R.; Ginebreda, A. J. Chem. Educ.1985, 62, 832.

A gas kinetic explanation of simple thermodynamic processesWaite, Boyd A.Proposes a simplified, semi-quantitative description of heat, work, and internal energy from the viewpoint of gas kinetic theory; both heat and work should not be considered as forms of energy but rather as different mechanisms by which internal energy is transferred from system to surroundings.Waite, Boyd A. J. Chem. Educ.1985, 62, 224.

Gases |

Kinetic-Molecular Theory |

Thermodynamics

Invisible water: A gas density demonstrationMaciel, Richard P.Demonstrating the density of 1,1,2-trichloro-1,2,2-trifluoroethane (TTE), whose density is about six times that of air.Maciel, Richard P. J. Chem. Educ.1985, 62, 153.

Gases |

Physical Properties

What a smell!Perkins, RobertHow many molecules of vanillin are necessary in order to smell it anywhere within the Goodyear Airship hangar?Perkins, Robert J. Chem. Educ.1984, 61, 384.

Gases |

Stoichiometry

Cooking with chemistryGrosser, Arthur E.Two demonstrations involving cooking eggs and suggestions for many more examples of cooking that illustrate important principles of chemistry. From the "State-of-the-Art Symposium for Chemical Educators: Chemistry of the Food Cycle".Grosser, Arthur E. J. Chem. Educ.1984, 61, 362.

Enduring distributions that deny BoltzmannNash, Leonard K.Examines two practical steady- state distributions: the atmosphere and its lapse rate and the ocean and its vertical quasi-uniformity.Nash, Leonard K. J. Chem. Educ.1984, 61, 22.

Atmospheric Chemistry |

Gases

Boyle's law experimentHermens, Richard A.This experiment regarding Boyle's law adheres to qualifications which allow the experiment to be meaningful to the students, is safe and simple to perform, low in cost, easy to set up and maintain, obtains reproducible results, and is capable of being performed in a reasonable length of time.Hermens, Richard A. J. Chem. Educ.1983, 60, 764.

Gases

Reflections upon mathematics in the introductory chemistry courseGoodstein, Madeline P.It is the purpose of this paper to call attention to the lack of mathematical competence by chemistry students and to invite consideration of one conceptual scheme which may be used to unify the mathematical approach.Goodstein, Madeline P. J. Chem. Educ.1983, 60, 665.

Chemometrics |

Gases

NH4HC03: a stimulant for learningRichards, R. RonaldStudents, professors, and the literature have all been confused by the unusual dissociation equilibrium of NH4HCO3.Richards, R. Ronald J. Chem. Educ.1983, 60, 555.

An effective demonstration of some properties of real vaporsMetsger, D. ScottThe apparatus described in this article has been found by the authors to be the most effective in vividly illustrating the behavior of a nearly ideal gas to first year chemistry students.Metsger, D. Scott J. Chem. Educ.1983, 60, 67.

Boyle's law - A different viewSharma, B. D.For a fixed mass of gas at constant temperature the energy of the gas is fixed and independent of its pressure and volume.Sharma, B. D. J. Chem. Educ.1982, 59, 827.

Pressure and the exploding beverage container Perkins, Robert R.The question in this article is an extension of exploding pop bottles to illustrate the balancing of a chemical equation, enthalpy, stoichiometry, and vapor pressure calculations, and the use of the Ideal Gas Equation. The question is aimed at the first-year level student.Perkins, Robert R. J. Chem. Educ.1981, 58, 363.

Balloons and the teaching of chemistryDewhurst, F.; Dewhurst, F. R.Balloons are a remarkably useful tool for the chemical educationalist. Balloons can not only provide cheap, safe, and easy-to-use alternatives to more complex and costly equipment, but also they can be used as effective teaching aids to demonstrate principles of structural chemistry.Dewhurst, F.; Dewhurst, F. R. J. Chem. Educ.1981, 58, 44.

A chemistry lesson at Three Mile IslandMammano, Nicholas J.Teaching principles of general chemistry through references made to the nuclear incident at Three Mile Island.Mammano, Nicholas J. J. Chem. Educ.1980, 57, 286.

Ga(U)Ge pressure and absolute pressureDavenport, Derek A.Air is progressively removed from a test tube; the pressure inside is measured using a standard tire-pressure gauge that is found to read atmospheric pressure when the test tube is fully evacuated.Davenport, Derek A. J. Chem. Educ.1979, 56, 322.

Gases

Boyle's lawDavenport, Derek A.Increasing weights are placed on a sealed syringe, compressing the air inside, and increasing weights pull the plunger from a held syringe, expanding the air inside. In both cases, plots of "P" vs. V are recorded.Davenport, Derek A. J. Chem. Educ.1979, 56, 322.

A discovery experiment. CO2 soap bubble dynamicsMillikan, Roger C.Students often make a choice of major based upon the view of a subject that they derive from the beginning course. Rare are the chemistry courses that provide the excitement and chance for discovery, while providing a basic understanding of chemistry. This article describes an experiment that does provide such an opportunity.Millikan, Roger C. J. Chem. Educ.1978, 55, 807.

Bubble pressure and volume. A demonstration experimentChristian, Sherril D.; Enwall, EricAn interesting phenomenon which illustrates several important principles, is the dependence of the size of a soap bubble on pressure. The subject is introduced to the class by the black box experiment presented in this article.Christian, Sherril D.; Enwall, Eric J. Chem. Educ.1978, 55, 536.

Gases |

Surface Science

Pressure calculations Schultz, Charles W.This question requires students to be able to distinguish two kinds of pressure: Boyles law pressure of gas (that depends on volume) from the equilibrium vapor pressure above a liquid (that does not).Schultz, Charles W. J. Chem. Educ.1978, 55, 515.

Gases |

Chemometrics

Teaching the method of successive approximationsNassiff, Peter J.; Boyko, E. R.The purpose of this papers is to help the teacher show the student why basic methods of successive approximations work, how they may be applied, and under what conditions it will be successful.Nassiff, Peter J.; Boyko, E. R. J. Chem. Educ.1978, 55, 376.

Great spray can debateBassow, HerbA curriculum scenario that takes the problems raised by the technological, economic, and political contexts of the fluorocarbon controversy as its point of focus.Bassow, Herb J. Chem. Educ.1977, 54, 371.

Atmospheric Chemistry |

Gases |

Enrichment / Review Materials |

Applications of Chemistry

Simplified Boyle's Law demonstrationMiller, Daniel W.Placing a sealed syringe in bell jar attached to a vacuum pump and reading the volume of air inside the syringe at various reduced pressures.Miller, Daniel W. J. Chem. Educ.1977, 54, 245.

Gases

Le Chtelier's principle: A laboratory exerciseFriedman, FredericaLe Chtelier's principle can be demonstrated by showing that water can boil at temperatures below 100C due to reduced vapor pressure.Friedman, Frederica J. Chem. Educ.1977, 54, 236.

Lab safety: The case of the errant cylinder Ozaruk, N.The anchoring of compressed gas cylinders to keep them from being knocked over, with the accompanying possibility of breaking off the valve, is an accepted safe practice. However, there has been some skepticism as to what would have happened if a cylinder valve was knocked off. The author shares a vivid description that appeared in the National Safety Council Chemical Section Newsletter. Also: a high school safety rules booklet; a hazardous materials safety booklet; and wall charts on Laboratory Techniques and Laboratory Safety.Ozaruk, N. J. Chem. Educ.1976, 53, 373.

A Dalton's law experiment for students in the health sciencesFeigl, Dorothy M.The number of students who take an introductory chemistry course in preparation for the health sciences is increasing. This note is an illustration of Dalton's law of partial pressures adapted to demonstrate the ability of the lungs to effect the removal of excess dioxide from the body.Feigl, Dorothy M. J. Chem. Educ.1974, 51, 273.

Tire Inflation ThermodynamicsPlumb, Robert C.; Connors, John J.Explains why inflating a tire with a hand pump heats the air being pumped into the tire.Plumb, Robert C.; Connors, John J. J. Chem. Educ.1971, 48, 837.

Gases |

Thermodynamics |

Applications of Chemistry

Bag-assembly for gas experimentGregory, MichaelAn improved bag-assembly has been devised for use with the Chem Study Experiment, "The Weights of Equal Volumes of Gases."Gregory, Michael J. Chem. Educ.1971, 48, 796.

Prolonging death (in apples)Plumb, Robert C.Using controlled atmosphere storage to prolong the freshness of vegetables and fruits after they have been harvested.Plumb, Robert C. J. Chem. Educ.1970, 47, 518.

Sealed tube experimentsCampbell, J. A.Lists and briefly describes a large set of "sealed tube experiments," each of which requires less than five minutes to set-up and clean-up, requires less than five minutes to run, provides dramatic results observable by a large class, and illustrates important chemical concepts.Campbell, J. A. J. Chem. Educ.1970, 47, 273.

Thermodynamics |

Crystals / Crystallography |

Solids |

Liquids |

Gases |

Rate Law |

Equilibrium

Cloud Caps on High MountainsStevenson, Philip E.The formation of cloud caps on high mountains illustrates cooling in an adiabatic expansion and the change in vapor pressure of a liquid with temperature.Stevenson, Philip E. J. Chem. Educ.1970, 47, 272.

Atmospheric Chemistry |

Gases |

Applications of Chemistry |

Phases / Phase Transitions / Diagrams |

Thermodynamics

A lecture-laboratory experiment in gas-liquid partition chromatographyMcKay, Edward S.; Vasers, AliseAfter being introduced to the chromatographic process in lecture, each student is given a copy of a chromatogram of an unknown mixture and asked to identify its composition and the concentration of each component.McKay, Edward S.; Vasers, Alise J. Chem. Educ.1970, 47, 239.

An improved equivalent weight apparatusBrown, Oliver L.Presents an improved apparatus for the reaction of weighed samples of metals with hydrochloric acid and the measurement of the volume of hydrogen evolved.Brown, Oliver L. J. Chem. Educ.1969, 46, 617.

Friday experimentsBissey, Jack E.Provides data on an unknown gas and asks readers to determine if it is ideal, as well as its molecular weight and chemical formula.Bissey, Jack E. J. Chem. Educ.1969, 46, 497.

Chemical queries. Especially for introductory chemistry teachersYoung, J. A.; Malik, J. G.; Bolte, John(1) Is the mole a number or a weight? (2) Is there an easy way to locate a compound by volume and page in Beilstein? (3) What are the stages evident in a gas discharge tube as the pressure of the gas and the voltage are changed? - answer by BolteYoung, J. A.; Malik, J. G.; Bolte, John J. Chem. Educ.1968, 45, 718.

Structure units: Aids in the interpretation of chemical reactionsStrong, Laurence E.the proposal to define structure units as generators of the various properties of a substance has a considerable advantage over the usual definition of a structure unit as the endpoint of some prescribed scheme of subdivision.Strong, Laurence E. J. Chem. Educ.1968, 45, 51.

Learning Theories |

Molecular Properties / Structure |

Solids |

Liquids |

Gases

The range of validity of Graham's LawsKirk, A. D.It is the purpose of this article to discuss effusion, diffusion, and some related processes and to outline the range of validity of Graham's law.Kirk, A. D. J. Chem. Educ.1967, 44, 745.

Gases |

Transport Properties

Graham's Laws of diffusion and effusionMason, E. A.; Kronstadt, BarbaraThe purpose of this article is to review Graham's laws of diffusion and effusion, offer simple but essentially correct theoretical explanations for both laws, and to present experiments on the diffusion law.Mason, E. A.; Kronstadt, Barbara J. Chem. Educ.1967, 44, 740.

An experimental approach to the ideal gas lawBreck, W. G.; Holmes, F. W.It is possible to introduce to students the equation of state, PV = nRT, by an experimental method that demonstrates that PV/T remains constant for a given amount of gas.Breck, W. G.; Holmes, F. W. J. Chem. Educ.1967, 44, 293.

The relationship between Avogadro's Principle and the Law of Gay-LussacFeifer, NathanTeaching Avogadro's Principle as an explanation of the phenomena described by Gay-Lussac's Law gives the instructor an opportunity to stress some of the basic assumptions in chemistry and to highlight the logic implicit in Avogadro's reasoning.Feifer, Nathan J. Chem. Educ.1966, 43, 411.

Kinetic energies of gas moleculesAherne, John C.The graph representing the distribution of kinetic energy among the molecules of a gas found in many textbooks is incorrect.Aherne, John C. J. Chem. Educ.1965, 42, 655.

Kinetic-Molecular Theory |

Gases

Determination of Avogadro's number by Perrin's lawSlabaugh, W. H.The experimental procedure for determining Avogadro's number by the Perrin method includes preparing a monodisperse colloid, ascertaining the mass of the particles, and making an accurate count of the number of particles at two points in the equilibrated colloid.Slabaugh, W. H. J. Chem. Educ.1965, 42, 471.

Maximum work revisited (Letters)Mysels, Karol J.Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.Mysels, Karol J. J. Chem. Educ.1964, 41, 677.

Thermodynamics |

Gases

Maximum work revisited (Letters)Bauman, RobertComments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.Bauman, Robert J. Chem. Educ.1964, 41, 676.

Thermodynamics |

Gases

Maximum work revisited (Letters)Kokes, Richard J.Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.Kokes, Richard J. J. Chem. Educ.1964, 41, 675.

Thermodynamics |

Gases

Maximum work revisited (Letters)Bauman, RobertComments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.Bauman, Robert J. Chem. Educ.1964, 41, 675.

The chemistry of the noble gasesHyman, Herbert H.Summarizes the chemistry of the noble gases and their bond-forming abilities.Hyman, Herbert H. J. Chem. Educ.1964, 41, 174.

Gases |

Main-Group Elements |

Covalent Bonding

Work of compressing an ideal gasBauman, Robert P.In formulating examples of compression problems there should be an explicit statement that the process is reversible, or at least slow.Bauman, Robert P. J. Chem. Educ.1964, 41, 102.

Thermodynamics |

Gases

Demonstration notes: Oxygen in airGlanz, JosephExplains that the popular method of demonstrating the percentage volume of oxygen in air is fraut with errors.Glanz, Joseph J. Chem. Educ.1963, 40, A477.

A simple gas law apparatusCarter, K. N.The apparatus presented here can be used to verify the ideal gas law, determine the vapor pressure of water at an elevated temperature, or determine the number of moles of dry air under two different sets of conditions for comparison.Carter, K. N. J. Chem. Educ.1962, 39, 302.

Laboratory Equipment / Apparatus |

Gases

Dalton's law of partial pressuresDutton, Frederic B.Demonstrates that breaking a sealed ampule of ether in a closed system increases the pressure inside that system.Dutton, Frederic B. J. Chem. Educ.1961, 38, A545.

Kinetic molecular theory from a jukeboxEasley, W. K.; Powers, Glenn F.Uses dancers to various styles of music as an analogy for differences between the atomic and molecular motions in solids, liquids, and gases.Easley, W. K.; Powers, Glenn F. J. Chem. Educ.1960, 37, 302.

Kinetic-Molecular Theory |

Solids |

Liquids |

Gases

Vapor pressure determination: An elementary experimentRadley, Edward T.The approximate vapor pressure of low boiling liquids may be estimated by measuring the increase in length of an air column trapped between two short columns of mercury in a uniform diameter tube.Radley, Edward T. J. Chem. Educ.1960, 37, 35.

A test tube automatic gas generatorAlpern, D. K.A simple design for an automatic gas generator can be used to produce common gases such as hydrogen from zinc and hydrochloric acid.Alpern, D. K. J. Chem. Educ.1959, 36, 302.

Laboratory Equipment / Apparatus |

Gases

The hydrogen organEddy, Robert D.The hydrogen organ can be used to demonstrate a variety of physical and chemical properties.Eddy, Robert D. J. Chem. Educ.1959, 36, 256.

Gases

Textbook errors: XX. Miscellanea No. 2Mysels, Karol J.Subjects considered include the meaning of "element," the solubility of phenol in carbonate solutions, and the change of vapor pressure with temperature.Mysels, Karol J. J. Chem. Educ.1958, 35, 568.

Le Châtelier's principle and the equilibrium constantMiller, Arild J.Many students of chemistry have difficulty in understanding how the position of equilibrium in a gaseous reaction can change when the pressure is altered, in accordance with Le Châtelier's principle, without causing a corresponding variation in the equilibrium constant.Miller, Arild J. J. Chem. Educ.1954, 31, 455.

Determination of the density of oxygen gasFiekers, B. A.The "Oxybomb," a small cartridge of compressed oxygen, is used for determining the density of oxygen gas in laboratory or lecture.Fiekers, B. A. J. Chem. Educ.1954, 31, 139.

The kinetic structure of gasesSlabaugh, W. H.Describes a model that illustrates the kinetic properties of gases and ii use to demonstrate the effect of temperature changes on the motion of gas particles.Slabaugh, W. H. J. Chem. Educ.1953, 30, 68.

Lettersde Milt, ClaraThe author calls for a mnemonic device to assist students in learning the gas laws and points out the omission of Graham's law from a recent textbook.de Milt, Clara J. Chem. Educ.1951, 28, 115.